Finding The Formula Of A Hydrate Lab

The purpose of the lab was to determine the percent of water in the hydrate MgSO4 * N2H0 through the process of heating the hydrate, releasing the water molecules, and leaving only the anhydrous magnesium sulfate and also determine the number of water molecules in the hydrate. Throughout the lab, various masses were tooki, including the mass of the evaporating glass with the watch glass, the mass of the evaporating glass, and watch glass with the additional hydrate sample, and the mass of the the evaporating glass, and the watch glass with the dehydrated sample, at two different times, each separated by a five minute interval. After, calculations based on the mass of the left over anhydrous solution were made where the mass of the either the original recorded number for the hydrate was used, or the aftermath dehydrated value of the hydrate. Soon the mass converted

This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next

The purpose of this lab is to determine the percent of water in a hydrate. I learned that copper sulfate hydrate is blue on its own but, when heat is added it will change color to a dim gray. One error that may have occurred is the failure to zero the scale which would ultimately change the math in the equation. Another error that may occur in this lab is forgetting to wait the recommended amount of cooling time, which would change the mass of the elements. At the end if the lab when we look to the questions, it is also beneficial to look at the notes for the lab because it helps with the setup of equations that may come with the questions, also it is very helpful

Finally, we measured the mass of the remaining copper in the test tube. This lead to the discovery that the mass of the copper in relation to our original 1.08 grams of copper oxide was 0.96 grams. From this data, we could find that the measurement of oxygen in our amount of copper oxide was 0.12 grams. With these significant weights, we were then able to convert those results to the amount of moles each element had in contribution to our total quantity of copper oxide. Specifically, we found that there was 0.015 moles of copper in our copper oxide, and 0.0075 moles of oxygen. So, that made the calculated ratio between moles of copper and moles of oxygen to be 2.0, or a 2:1 ratio of copper to oxygen. Thus, the formula of the red copper oxide can be expressed as . The lab worked the way it did primarily because of the chemical characteristics of copper oxide. Since the oxygen could separate from the copper when presented with a heat source, it allowed for the amount of each element in our quantity of copper oxide to be measured and then calculated into a ratio, which determined the formula for the

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

The primary of this lab is about the hydrate. The hydrate is a compound formed by an ionic bond combined with the water molecule (known as “water of hydration”) attached to it. So for every formula unit, there would be some amount of water molecule combined with the ionic compound and would act as a single compound. Our theoretical hydrate for this lab was CuSO4 * 5H2O. To remove the water from the compound and get the mass of the ionic compound, you need to follow the dehydrating procedure by heating. That would separate the ionic bond (CuSO4) from the water molecule (5H2O) once it reaches certain decomposition temperature. And to physically determine whether or not the water of hydration is removed, see the color, in our case, turning white from blue. Once the water molecules have entirely evaporated, the mass left would be the weight of the ionic compound (mass of CuSO4 in grams).

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

3) Repeat the drying process just to be sure that the copper is completely dry, and again determine the mass of the copper and the beaker.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

Weigh out the necessary grams of Copper Sulfate Pentahydrate. The 40-degree group weighed out 40 grams. (See Figure 1)

Another run 2 was made and the set-up where the reaction will take place was ensured to be at room temperature. 4 drops of CuSo4 was added immediately after Beaker A was poured to Beaker B. The reaction was timed until it turned to blue.

Solutions of CuSO45H2O (0.506 g in 10mL water, 3.17E-3 mol) and ammonium peroxodisulfate (1.030 g in 10mL water, 4.51E-3 mol) were prepared and mixed

0.5% of copper sulphate solution was added by drop at a time and and the test tube was shaked continuously.